Electrolysis and Faraday's Law Practice Test

Molten sodium chloride is electrolyzed, producing sodium metal at the cathode according to $\text{Na}^+ + e^- \rightarrow \text{Na}(l)$. If a constant current of $4.00\ \text{A}$ is applied for $20.0\ \text{min}$, what mass of $\text{Na}$ is produced? (Assume 100% current efficiency.)

Molten sodium bromide, $\text{NaBr}(l)$, is electrolyzed. The current is $4.82\ \text{A}$ for $2.00\times 10^3\ \text{s}$. At the anode, bromine is produced according to $2\text{Br}^-\rightarrow \text{Br}_2(g)+2e^-$. Assuming 100% current efficiency, what amount of $\text{Br}_2(g)$ is produced?